1. Chemistry Chapter 3
Atoms:
The Building
Blocks of Matter

2. Law of Conservation of Mass
Atom who?
Atom
The ________ particle of an element that retains the _____________ of that element
Law of Conservation of Mass
Mass is neither _________ __________ during chemical or physical reactions.
Total mass of __________ =
Antoine Lavoisier

3. Dalton’s Atomic Theory (1808)
All matter is composed of extremely small particles called ________.
Atoms of a given element are ________ in size, mass, and other properties; atoms of __________ elements differ in size, mass, and other properties.
John Dalton
Atoms ________ be subdivided, created, or destroyed.
Atoms of different elements combine in simple ________________ to form chemical compounds.
In _____________, atoms are combined, separated, or rearranged.

4. Modern Atomic Theory Changes have been made to Dalton’s theory..
Dalton said:
Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties
Modern theory states:
Atoms of an element have a characteristic ___________ which is unique to that element.
Dalton said:
Atoms cannot be subdivided, created, or destroyed
Modern theory states:
Atoms cannot be subdivided, created, or destroyed in __________________. However, these changes CAN occur in nuclear reactions!

5. Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube to deduce the presence of a _________ charged particle.
Cathode ray tubes pass __________ through a gas that is contained at a very low pressure.

6. _____________and the charge is _____________
Mass of the Electron
1909 – Robert Millikan determines the mass of the electron.
The oil drop apparatus
Mass of the electron is
_____________and the charge is _____________
An experiment performed by Robert Millikan in 1909 determined the size of the charge on an electron. He also determined that there was a smallest 'unit' charge, or that charge is 'quantized'. He received the Nobel Prize for his work. We're going to explain that experiment here, and show how Millikan was able to determine the size of a charge on a single electron.
What Millikan did was to put a charge on a tiny drop of oil, and measure how strong an applied electric field had to be in order to stop the oil drop from falling. Since he was able to work out the mass of the oil drop, and he could calculate the force of gravity on one drop, he could then determine the electric charge that the drop must have. By varying the charge on different drops, he noticed that the charge was always a multiple of -1.6 x C, the charge on a single electron. This meant that it was electrons carrying this unit charge. Here's how it worked. Have a look at the apparatus he used:
An atomizer sprayed a fine mist of oil droplets into the chamber. Some of these tiny droplets fell through a hole in the upper floor. Millikan first let them fall until they reached terminal velocity. Using the microscope, he measured their terminal velocity, and by use of a formula, calculated the mass of each oil drop. Next, Millikan applied a charge to the falling drops by illuminating the bottom chamber with x-rays. This caused the air to become ionized, and electrons to attach themselves to the oil drops. By attaching a battery to the plates above and below this bottom chamber, he was able to apply an electric voltage. The electric field produced in the bottom chamber by this voltage would act on the charged oil drops; if the voltage was just right, the electromagnetic force would just balance the force of gravity on a drop, and the drop would hang suspended in mid-air. Now you try it. Click here to open a simulation of Millikan's chamber. First, allow the drops to fall. Notice how they accelerate at first, due to gravity. But quickly, air resistance causes them to reach terminal velocity. Now focus on a single falling drop, and adjust the electric field upwards until the drop remains suspended in mid-air. At that instant, for that drop, the electric force on it exactly equals the force of gravity on it. Some drops have more electrons than others, so will require a higher force to stop. When you've finished playing with the apparatus, close the window and we'll continue. O.K., let's look at the calculation Millikan was now able to do. When a drop is suspended, its weight  m · g is exactly equal to the electric force applied  q · E
The values of  E, the applied electric field,  m the mass of a drop, and  g, tha acceleration due to gravity, are all known values. So you can solve for  q, the charge on the drop:
Millikan determined the charge on a drop. Then he redid the experiment numerous times, each time varying the strength of the x-rays ionizing the air, so that differing numbers of electrons would jump onto the oil molecules each time. He obtained various values for  q. The charge  q on a drop was always a multiple of -1.6 x C,  the charge on a single electron. This number was the one Millikan was looking for, and it also showed that the value was quantized; the smallest unit of charge was this amount, and it was the charge on a single electron.

7. Conclusions from the Study of the Electron
Electrons are ___________.
Cathode rays have _________ properties regardless of the element used to produce them. All elements must contain _________ charged electrons.
Atoms are ________, so there must be ________ particles in the atom to balance the ________ charge of the electrons
Electrons have so ______ mass that atoms must contain other particles that account for most of the mass

8. Rutherford’s Gold Foil Experiment
Alpha particles are ________ charged
Particles were fired at a thin sheet of gold foil
Particle hits on the detecting screen (film) are recorded

9. Rutherford’s Findings
_____ of the particles passed right through
A _____ particles were deflected
VERY ______ were greatly deflected
Conclusions:
The nucleus is ______
The nucleus is _____
The nucleus is ________ charged

10. The Structure of the Atom
Atoms consist of two regions
_________
Very small region in the center.
Contains protons & neutrons (nucleons).
__________
Mainly empty space.
Very large compared to the nucleus.
Contains electrons.
Subatomic particles
Particle
Charge
Mass (kg)
Location
Electron
9.109 x 10-31
Electron cloud
Proton
1.673 x 10-27
Nucleus
Neutron
1.675 x 10-27

11. Atomic Number Mass Number
Atomic number (Z) of an element is the number of ________ in the nucleus of each atom of that element. Identifies the atom.
Mass Number
Mass number is the number of _______ and ________ in the nucleus of an isotope.
Mass # = p+ + n0
Nuclide p+ n0 e-
Mass #
Oxygen - 10 - 33 42
- 31 15

12. Isotopes Elements occur in nature as mixtures of isotopes.
Isotopes are atoms of the __________ that differ in the number of _______

13. Isotopes…Again (must be on the test)
Isotopes are atoms of the same element having different masses due to varying numbers of neutrons.
Isotope
Protons
Electrons
Neutrons
Nucleus
Hydrogen–1 (_______)
Hydrogen-2 (________)
Hydrogen-3 (______)

14. Atomic Masses
Atomic mass is the ________ of all the naturally isotopes of that element.
On Periodic Table
Carbon =
Isotope
Symbol
nucleus
% in nature
Carbon-12
12C
6 protons
6 neutrons
98.89%
Carbon-13
13C
7 neutrons
1.11%
Carbon-14
14C
8 neutrons
<0.01%

15. Writing Nuclear Symbols3 He
Mass #
(____________)
Atomic Symbol
Atomic #
(_______) 2
How many protons, electrons, and neutrons?

16. Writing Isotopes Using Hyphen Notation
Uranium-235, Helium-3, or Carbon-14
How many proton, electrons, neutrons?
Name
of atom
Mass #

17. Convert these hyphen notation to nuclear symbols.
Isotope problems
Convert these hyphen notation to nuclear symbols.
Uranium-235, Helium-3, or Carbon-14

18. The Nucleus Contains nucleons _____________ ________________
Short-range proton-neutron, proton-proton, and neutron-neutron forces hold the nuclear particles together.

19. Nuclear Stability
Decay will occur in such a way as to return a nucleus to the band (line) of stability.
Kinetic Stability describes the probability that a nucleus will decompose (radioactive decay)

20. Number of Stable Nuclides Related to Numbers of Protons and Neurons

21. Types of Radioactive Decay
alpha production (a): helium nucleus _____
beta production (b): _____

22. Types of Radioactive Decay
gamma ray production (g):
positron production :
electron capture: (inner-orbital electron is captured by the nucleus) e 1

23. Types of Radiation

24. The Decay of a 10.0-g Sample of Strontium-90 Over Time

25. QUESTIONS

26. QUESTIONS